The Average Rate of a Reaction
|
|
- Cassandra Francis
- 7 years ago
- Views:
Transcription
1 Kinetics The main factors that affect the rate of a chemical reaction are temperature, concentration, pressure and surface area which you have covered in AS. What is a reaction rate? Well if you take the example reaction: A + 2B C The concentrations of A and B will decrease with time, and C will increase with time. We could plot our results like so: The rate of reaction is defined as the change in concentration (of any of the reactants or products) with time. Notice though how different the graphs for each one is, which means that you need to state which one you are following. In most cases you will follow C, as this is your product, and it will increase with time A B C
2 The Average Rate of a Reaction We can find an average rate from a graph of concentration against time. The average rate of the reaction with respect to C, during a period of time Dt is the change in concentration of C divided D[C] by Dt. The average rate of reaction between t 1 and t 2 = D[C] / Dt Therefore if in 10 seconds [C] changed from 1.0mol dm -3 to 1.1mol dm -3 then: mol dm -3 = Average rate of reaction in this period 10s = 0.1 / 10 = 1x10-2 mol dm -3 s -1
3 The rate of reaction at any instant Quite often it is more useful for us to know the rate of reaction over a certain period of time. To find the rate of change of [C] at a particular instant we draw a tangent to the curve at that time and then find the gradient or slope.
4 Measuring a reaction rate To measure the reaction rate we need a method to do this. This method will be different depending on the reaction that is taking place and how quickly this happens. Example: The reaction of Bromine and Methanoic acid. The solution starts off being brown and ends up being colourless. Br 2 (aq) + HCO 2 H(aq) 2Br - (aq) + 2H + (aq) + CO 2 (g) For this particular reaction we use a colorimeter, which can measure the decreasing concentration of Br 2. This relies on the Beer-Lambert Law which says that the absorption of light by a particular substance is due to the properties of the substances that it is passing through. It takes into account values such as the length of the path of light and concentration of the compound in solution.
5 Colorimeter The essential parts of a colorimeter are: a light source (often an ordinary low-voltage filament lamp) an adjustable aperture a set of colored filters a cuvette to hold the working solution a detector (usually a photoresistor) to measure the transmitted light a meter to display the output from the detector In addition, there may be: a voltage regulator, to protect the instrument from fluctuations in mains voltage. a second light path, cuvette and detector. This enables comparison between the working solution and a "blank", consisting of pure solvent, to improve accuracy.
6 Reaction between Bromine and Methanoic Acid Time (s) [Br 2 ] mol dm
7 Reaction between Bromine and Methanoic Acid Find the rate t = 0s t = 300s t = 500s
8 Reaction between Bromine and Methanoic Acid Answers: t = D[C] / Dt 1. t = / 215 = 4.000x10-5 mol dm-3 s-1 2. t = / 585 = 1.196x10-5 mol dm-3 s-1 3. t = / 750 = 7.066x10-6 mol dm-3 s-1
9 The rate expression and order of reaction The rate of a reaction depends on the concentrations of some or all of the species in the reaction vessel (reactants, products and catalysts). They will not always make the same contribution to the reaction rate. The rate expression will tell us about the contribution of the species that DO affect the reaction rate. Example: X + Y Z The concentration of X [X], may have more effect on the rate than the concentration of Y [Y]. It could also be that the [X] has NO effect on the rate, or even that [Z] has an effect. All of this information can be found by experimental procedures.
10 The rate expression The rate expression describes how the rate of the reaction depends on the concentration of species involved in the reaction. All the reactants may not appear in the rate expression, this is because these particular species have no effect on the rate. For example: The rate expression for X + Y Z may have the rate expression [X][Y] where means proportional to. This would mean that both [X] and [Y] have an equal effect on the rate. Doubling either one of these would double the rate of reaction. Doubling the concentration of both would quadruple the rate. It could be that the rate expression is [X][Y] 2 This would mean that doubling [X] would double the rate of reaction but doubling [Y] would quadruple the rate.
11 The rate constant k We can remove the proportionality sign if we introduce a constant to the expression. This constant is k and is different for every reaction and varies with temperature, so the temperature needs to be stated. If the concentration of all the species is 1 mol dm -3 then the rate of reaction is k. Therefore if the rate expression were [X][Y] 2 This can be written as k[x][y] 2
12 The order of a reaction Take the rate equation: Rate = k[x][y] 2 This means that [Y], which is raised to the power of 2, has double the effect on the rate than that of [X]. The order of reaction with respect to one of the species, is the power to which the concentration of that species is raised to. It tells us how the rate depends on the concentration of that species. So for our particular example the order of reaction with respect to Y is two and to X is one. The overall order of reaction would be the sum of the orders of all the species. So this reaction is first order in respect to X, second order in respect to Y and third order overall.
13 Chemical equations and the rate equation The rate equations tells us about the species which affect the rate. The species in a chemical equation may not appear in the rate equation, also the coefficient of a species in the chemical equation has no relevance on the rate expression. For example: CH 3 COCH 3 (aq) + I 2 (aq) CH 2 ICOCH 3 (aq) + HI(aq) After experiment, the rate equation was found to be: Rate = k[ch 3 COCH 3 (aq)] [H + (aq)] So we could say that this reaction is first order in respect to propanone, first order in respect to H + ions and second order overall. The rate is zero order in respect to iodine or [I] 0.
14 Units of the rate constant, k The units of the rate constant varies depending on the overall order of reaction. For a first order reaction, such as: Rate = k[a] The units of rate are mol dm -3 s -1 and the units of [A] are mol dm -3 so the units of k are s -1. Therefore if you cancel out the units: mol dm -3 s -1 = k x mol dm -3 == k = mol dm -3 s -1 / mol dm -3 Therefore the unit of k for a first order reaction is s -1. Another example, this time for a second order reaction: Rate = k[b][c] mol dm -3 s -1 = k x mol dm -3 x mol dm -3 == k = mol dm -3 s -1 / mol dm -3 x mol dm -3 Therefore the unit of k for a second order reaction is mol -1 dm 3 s -1
15 Finding the order of reaction from a graph The results from most reaction rate experiments will give you a series of concentration readings for one particular species. Usually the first step to finding the order with respect to that species is by plotting these readings on a concentration time graph. To help the interpretation of the experiment, we make sure that the concentrations of all the reactants, other than the one being measured, stay the same. We do this by making their concentration so large compared with the reactant being Investigated, that any change is negligible. Example: Reactant R R + B Products Reactant B At the start of the reaction we make [B] very large compared with [R]. For example: At the start: [R] = 0.01 mol dm-3 [B] = 1.00 mol dm-3 At the end: [R] = 0 (all used up) [B] = 0.99 mol dm-3 So during the whole reaction [B] is practically constant.
16 Finding the order of reaction from a graph The graph of [R] plotted against time will look different depending on the order. Zero Order First Order Second Order Notice that in all of the graphs the concentration of R decreases with time. This is because R is the reactant and is therefore is being used up. Just by looking at the graph can often tell you what the order of reaction is. If it is a straight line the order of reaction is zero, this is because the rate is the same whatever the concentration of R is. First and second order reactions both give curves by the second order is deeper than the first order one.
17 Finding the half-life of a first order reaction The half life of a reaction, t1/2, is the time take for [R] to fall from any chosen value to half that value. The first half-life is often taken from the start of the reaction. The second half-life is from the end of the first etc. In a first order reaction all the half lives are the same. For a second order reaction and greater, successive half lives increase.
18 Finding the order of a reaction by using rateconcentration graph Another way of determining the order of a reaction with respect to a particular species is by plotting a graph of rate against concentration (rather than concentration against time). We start off by drawing a usual graph of [R] against time and draw tangents at the different values of [R]. The gradients of these tangents are the reaction rates (changes in concentration over time) at different concentrations. The values for these rates can then be used to construct a second graph of rate against concentration. If the graph is a horizontal straight line, this means that the rate is unaffected by [R] so the order is zero. If this graph is a sloping straight line through the origin then rate is proportional [R] so the order is one. If the graph is not a straight line then it is probably second order. To prove this plot rate against [R] 2, if this is a straight line the it is second order.
19 The initial rate method The previous method we discussed allows us to find the order of reaction with respect to the one reactant whose concentration we measured. This method allows us to find the order of reactant with respect to any species in the reaction mixture. With this method a series of experiments are carried out, Each experiment starts with a different combination of initial concentrations of reactants, catalysts etc. The experiments are designed so that for any pair of experiments, there is only one concentration that varies, the rest stay the same. Then for each experiment, the concentration of one reactant is followed and the concentration-time graph plotted. On the graph a tangent at time=0 is drawn and the gradient of this line is the initial rate. The good thing about this method is that the concentrations of ALL the substances in the reaction mixture are known exactly at this time. Comparing the initial concentration and the initial rates for pairs of experiments allows the order with respect to each reactant to be found.
20 The initial rate method An example of this is the reaction: 2NO(g) + O 2 (g) 2NO 2 (g) Experiment Number Initial [NO]/10-3 mol dm-3 Initial [O 2 ]/10-3 mol dm Initial rate/10-4 mol dm-3 s-1 Comparing experiment 1 and 2: [NO] is doubled but [O 2 ] stays the same. The rate is shown to quadruple (7 28) which suggests rate [NO] 2. This can be confirmed by looking at experiment 1 and 3 where [NO] is trebled while [O 2 ] is kept the same. Here the rate increases nine fold as we would expect. So the order with respect to NO is two. Now you can compare experiment 2 and 4. Here [NO] is constant but [O 2 ] doubles. The rate doubles from (28 56) so it looks as if rate [O 2 ]. This can be confirmed by looking at experiments 3 and 5. Again [NO] is constant, but [O 2 ] triples. The rate triples too, confirming that the order in respect to [O 2 ] is one. Therefore: rate [NO] 2 rate [O 2 ] 1 rate [NO] 2 [O 2 ] 1 Provided that no other species affect reaction rate: rate = k [NO] 2 [O 2 ]
21 Finding the rate constant k To find k in the equation mentioned before, we simply substitute any set of values for rate, [NO] and [O2] in the equation. Remember to work the units out as well as the units for k change depending on the order of reaction. So taking the values for experiment 2: 28 x 10-4 = k x (2x10-3 ) 2 x (1 x 10-3 ) 28 x 10-4 = k x (4x10-9 ) 28 x 10-4 = 7x x 10-9 Now units: OVERALL: 7x10 5 mol -2 dm 6 s -1 mol dm -3 s -1 = k x mol 2 dm -6 x mol dm -3 mol dm -3 s -1 = mol -2 dm 6 s -1 mol 3 dm -9
22 The effect of temperature on k Small changes in temperature produce large changes in reaction rates. A rule of thumb is that for every 10K rise in temperature, the rate of reaction doubles. Suppose the rate expression for a reaction is rate = k [A][B]. We know that [A] and [B] do not change with temperature, so therefore the rate constant, k, must increase with temperature. The rate constant, k, is a measure of the speed of a reaction. The larger the value of k, the faster the reaction. k increases with temperature, and this is true for all reactions. You should already be aware that increasing the temperature increases reaction rate. You should also know that the reason for this is because raising the temperature will give colliding particles enough energy to start bond breaking, or giving them enough energy to overcome the E A (activation energy).
23 The rate determining step Most reactions take place in more than one step. The separate steps that lead from reactants to products are together called the reaction mechanism. For example look at the reaction below: BrO 3- (aq) 6H + (aq) + 5Br - (aq) 3Br 2 (aq) + 3H 2 O(l) The above reaction has 12 ions, the chances of these all hitting each other at the same time, and having enough energy is VERY slim. What happens is the steps in between have very short lived intermediates. The problem is, is these intermediates are usually impossible to isolate and identify, therefore we must find other ways of working out the mechanism.
24 The rate determining step In a multi step reaction the steps nearly always follow after each other, so that the product(s) of one step is/are the starting material(s) for the next. Therefore the slowest step is the one that governs the rate of the whole process. The slowest step forms a bottleneck called the rate determining step. In a chemical reaction, any step that occurs after the rate determining step will not affect the rate. The reason for this is as follows. Consider this expression: A + B + C Y + Z This could happen like this: 1. A + B D (FAST) 2. D E (SLOW) 3. E + C Y + Z Step 2 is the slowest step and so determines the rate. As soon as some E is produced it rapidly reacts with C to produce Y and Z. BUT the rate of step 1 might affect the overall rate the concentration of D depends on this. So any species involved before the rate-determining step could affect the rate and therefore appear in the rate expression.
25 The rate determining step The reaction between iodine and propanone. The rate expression is found to be: Rate=k [CH 3 OCCH 3 ][H + ] Various mechanisms could be proposed for this reaction. One of them is as follows:- Step 1 The propanone is protonated (picks up an H + ion) slow Step 2 This ion undergoes rearrangement and forms a C=C double bond fast Step 3 Iodine adds across the double bond fast Step 4 The carbonyl C=O bond is re-established by the elimination of a proton (restoring the catalyst) and an iodide ion fast
26 Step 1: slow Step 2: fast Step 3: fast H + + H 3 C C CH 3 H 3 C C+ CH 3 O OH H 3 C C+ CH 3 H 2 C C CH 3 OH OH I I I 2 + H 2 C C CH 3 H 2 C C CH 3 OH OH + H + Step 4: fast I H 2 C I C CH 3 C CH 3 OH O Step 1 is obviously the RDS and it involves only the propanone and the acid catalyst. The iodine molecules are not involved in the mechanism until later, so the overall rate does not depend on the concentration of iodine. This is consistent with the experimental evidence. It is important to realise, however, that the mechanistic suggestion above was not deduced from the kinetic evidence; the evidence was merely shown to be consistent with the suggestion. H 2 CI + H + + I -
1A Rate of reaction. AS Chemistry introduced the qualitative aspects of rates of reaction. These include:
1A Rate of reaction AS Chemistry introduced the qualitative aspects of rates of reaction. These include: Collision theory Effect of temperature Effect of concentration Effect of pressure Activation energy
More informationChemical Kinetics. 2. Using the kinetics of a given reaction a possible reaction mechanism
1. Kinetics is the study of the rates of reaction. Chemical Kinetics 2. Using the kinetics of a given reaction a possible reaction mechanism 3. What is a reaction mechanism? Why is it important? A reaction
More informationReaction Rates and Chemical Kinetics. Factors Affecting Reaction Rate [O 2. CHAPTER 13 Page 1
CHAPTER 13 Page 1 Reaction Rates and Chemical Kinetics Several factors affect the rate at which a reaction occurs. Some reactions are instantaneous while others are extremely slow. Whether a commercial
More informationThe relationship between the concentration of a reactant and the rate of reaction with respect to that reactant can be shown using rate time graphs.
The effect of concentration on rate Student sheet To study The relationship between the concentration of a reactant and the rate of reaction with respect to that reactant can be shown using rate time graphs.
More informationReaction of Blue Food Dye with Bleach
Exercise 2 Reaction of Blue Food Dye with Bleach 2 Introduction In the experiment, you will study the rate of the reaction of FD&C Blue #1 (Blue #1 is denoted by E number E133 in food stuff) with sodium
More informationChapter 12 - Chemical Kinetics
Chapter 1 - Chemical Kinetics 1.1 Reaction Rates A. Chemical kinetics 1. Study of the speed with which reactants are converted to products B. Reaction Rate 1. The change in concentration of a reactant
More informationIB Chemistry. DP Chemistry Review
DP Chemistry Review Topic 1: Quantitative chemistry 1.1 The mole concept and Avogadro s constant Assessment statement Apply the mole concept to substances. Determine the number of particles and the amount
More informationChemical Kinetics. Reaction Rate: The change in the concentration of a reactant or a product with time (M/s). Reactant Products A B
Reaction Rates: Chemical Kinetics Reaction Rate: The change in the concentration of a reactant or a product with time (M/s). Reactant Products A B change in number of moles of B Average rate = change in
More informationNuclear Structure. particle relative charge relative mass proton +1 1 atomic mass unit neutron 0 1 atomic mass unit electron -1 negligible mass
Protons, neutrons and electrons Nuclear Structure particle relative charge relative mass proton 1 1 atomic mass unit neutron 0 1 atomic mass unit electron -1 negligible mass Protons and neutrons make up
More informationChemistry B11 Chapter 4 Chemical reactions
Chemistry B11 Chapter 4 Chemical reactions Chemical reactions are classified into five groups: A + B AB Synthesis reactions (Combination) H + O H O AB A + B Decomposition reactions (Analysis) NaCl Na +Cl
More informationChapter 13 Chemical Kinetics
Chapter 13 Chemical Kinetics Student: 1. The units of "reaction rate" are A. L mol -1 s -1. B. L 2 mol -2 s -1. C. s -1. D. s -2. E. mol L -1 s -1. 2. For the reaction BrO 3 - + 5Br - + 6H + 3Br 2 + 3H
More informationAmount of Substance. http://www.avogadro.co.uk/definitions/elemcompmix.htm
Page 1 of 14 Amount of Substance Key terms in this chapter are: Element Compound Mixture Atom Molecule Ion Relative Atomic Mass Avogadro constant Mole Isotope Relative Isotopic Mass Relative Molecular
More informationEquilibria Involving Acids & Bases
Week 9 Equilibria Involving Acids & Bases Acidic and basic solutions Self-ionisation of water Through reaction with itself: The concentration of water in aqueous solutions is virtually constant at about
More informationNet ionic equation: 2I (aq) + 2H (aq) + H O (aq) I (s) + 2H O(l)
Experiment 5 Goals To determine the differential rate law for the reaction between iodide and hydrogen peroxide in an acidic environment. To determine the activation energy and pre-exponential factor for
More informationExperiment 2 Kinetics II Concentration-Time Relationships and Activation Energy
2-1 Experiment 2 Kinetics II Concentration-Time Relationships and Activation Energy Introduction: The kinetics of a decomposition reaction involving hydroxide ion and crystal violet, an organic dye used
More informationEXPERIMENT 2 THE HYDROLYSIS OF t-butyl CHLORIDE. PURPOSE: To verify a proposed mechanism for the hydrolysis of t-butyl Chloride.
PURPOSE: To verify a proposed mechanism for the hydrolysis of t-butyl Chloride. PRINCIPLES: Once the Rate Law for a reaction has been experimentally established the next step is its explanation in terms
More informationTest Review # 9. Chemistry R: Form TR9.13A
Chemistry R: Form TR9.13A TEST 9 REVIEW Name Date Period Test Review # 9 Collision theory. In order for a reaction to occur, particles of the reactant must collide. Not all collisions cause reactions.
More informationLab #11: Determination of a Chemical Equilibrium Constant
Lab #11: Determination of a Chemical Equilibrium Constant Objectives: 1. Determine the equilibrium constant of the formation of the thiocyanatoiron (III) ions. 2. Understand the application of using a
More informationPhenolphthalein-NaOH Kinetics
Phenolphthalein-NaOH Kinetics Phenolphthalein is one of the most common acid-base indicators used to determine the end point in acid-base titrations. It is also the active ingredient in some laxatives.
More informationph. Weak acids. A. Introduction
ph. Weak acids. A. Introduction... 1 B. Weak acids: overview... 1 C. Weak acids: an example; finding K a... 2 D. Given K a, calculate ph... 3 E. A variety of weak acids... 5 F. So where do strong acids
More informationTitration curves. Strong Acid-Strong Base Titrations
Titration curves A titration is a procedure for carrying out a chemical reaction between two solutions by the controlled addition from a buret of one solution (the titrant) to the other, allowing measurements
More informationCHAPTER 13 Chemical Kinetics: Clearing the Air
CHAPTER 13 Chemical Kinetics: Clearing the Air 13.1. Collect and Organize For the plot of Figure P13.1, we are to identify which curves represent [N O] and [O ] over time for the conversion of N O to N
More informationph: Measurement and Uses
ph: Measurement and Uses One of the most important properties of aqueous solutions is the concentration of hydrogen ion. The concentration of H + (or H 3 O + ) affects the solubility of inorganic and organic
More informationReaction Stoichiometry and the Formation of a Metal Ion Complex
Reaction Stoichiometry and the Formation of a Metal Ion Complex Objectives The objectives of this laboratory are as follows: To use the method of continuous variation to determine the reaction stoichiometry
More information20.2 Chemical Equations
All of the chemical changes you observed in the last Investigation were the result of chemical reactions. A chemical reaction involves a rearrangement of atoms in one or more reactants to form one or more
More informationChapter 14. Chemical Kinetics
14.1 Factors that Affect Reaction Rates Chemical kinetics = the study of how fast chemical reactions occur. Factors which affect rates of reactions: Physical state of the reactants. Concentration of the
More informationMath 231:Introduction to Ordinary Differential Equations Mini-Project: Modeling Chemical Reaction Mechanisms
Department of Mathematics Fall 2012 The University of Tennessee H. Finotti Math 231:Introduction to Ordinary Differential Equations Mini-Project: Modeling Chemical Reaction Mechanisms Chemical kinetics,
More information6 Reactions in Aqueous Solutions
6 Reactions in Aqueous Solutions Water is by far the most common medium in which chemical reactions occur naturally. It is not hard to see this: 70% of our body mass is water and about 70% of the surface
More informationChemistry 111 Lab: Intro to Spectrophotometry Page E-1
Chemistry 111 Lab: Intro to Spectrophotometry Page E-1 SPECTROPHOTOMETRY Absorption Measurements & their Application to Quantitative Analysis study of the interaction of light (or other electromagnetic
More informationElectrical Conductivity of Aqueous Solutions
Electrical Conductivity of Aqueous Solutions PRE-LAB ASSIGNMENT: Reading: Chapter 4.-4.3 in Brown, LeMay, Bursten & Murphy.. Using Table in this handout, determine which solution has a higher conductivity,.
More informationStudying an Organic Reaction. How do we know if a reaction can occur? And if a reaction can occur what do we know about the reaction?
Studying an Organic Reaction How do we know if a reaction can occur? And if a reaction can occur what do we know about the reaction? Information we want to know: How much heat is generated? How fast is
More informationVolumetric Analysis. Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115
Volumetric Analysis Lecture 5 Experiment 9 in Beran page 109 Prelab = Page 115 Experimental Aims To prepare and standardize (determine concentration) a NaOH solution Using your standardized NaOH calculate
More informationAP Chemistry 2010 Scoring Guidelines Form B
AP Chemistry 2010 Scoring Guidelines Form B The College Board The College Board is a not-for-profit membership association whose mission is to connect students to college success and opportunity. Founded
More informationChapter 14: Chemical Kinetics: Reactions in the Air We Breathe
Chapter 4: Chemical Kinetics: Reactions in the Air We Breathe Problems: 4.-4.9, 4.-4., 4.4, 4.6-4.33, 4.37, 4.4 Consider the formation of rust (or oxidation of iron). a. It can occur over a period of several
More informationIB Chemistry 1 Mole. One atom of C-12 has a mass of 12 amu. One mole of C-12 has a mass of 12 g. Grams we can use more easily.
The Mole Atomic mass units and atoms are not convenient units to work with. The concept of the mole was invented. This was the number of atoms of carbon-12 that were needed to make 12 g of carbon. 1 mole
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the ionic compounds NaF, CsI, and CaO in order of increasing lattice energy. Analyze From the formulas for three
More informationChapter 9 Lecture Notes: Acids, Bases and Equilibrium
Chapter 9 Lecture Notes: Acids, Bases and Equilibrium Educational Goals 1. Given a chemical equation, write the law of mass action. 2. Given the equilibrium constant (K eq ) for a reaction, predict whether
More informationMEMORANDUM GRADE 11. PHYSICAL SCIENCES: CHEMISTRY Paper 2
MEMORANDUM GRADE 11 PHYSICAL SCIENCES: CHEMISTRY Paper 2 MARKS: 150 TIME: 3 hours Learning Outcomes and Assessment Standards LO1 LO2 LO3 AS 11.1.1: Plan and conduct a scientific investigation to collect
More informationPaper 1 (7404/1): Inorganic and Physical Chemistry Mark scheme
AQA Qualifications AS Chemistry Paper (7404/): Inorganic and Physical Chemistry Mark scheme 7404 Specimen paper Version 0.6 MARK SCHEME AS Chemistry Specimen paper Section A 0. s 2 2s 2 2p 6 3s 2 3p 6
More informationHonors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1. A chemical equation. (C-4.4)
Honors Chemistry: Unit 6 Test Stoichiometry PRACTICE TEST ANSWER KEY Page 1 1. 2. 3. 4. 5. 6. Question What is a symbolic representation of a chemical reaction? What 3 things (values) is a mole of a chemical
More informationIII. Chemical Kinetics
WARNING NOTICE: The experiments described in these materials are potentially hazardous and require a high level of safety training, special facilities and equipment, and supervision by appropriate individuals.
More informationThe 5 Types of Chemical Reactions (Chapter 11) By C B 6 th period
The 5 Types of Chemical Reactions (Chapter 11) By C B 6 th period 1) Combination Reactions Is also referred to as a synthesis reaction It is a chemical change in which two or more substances react to form
More informationCHEMICAL EQUILIBRIUM (ICE METHOD)
CHEMICAL EQUILIBRIUM (ICE METHOD) Introduction Chemical equilibrium occurs when opposing reactions are proceeding at equal rates. The rate at which the products are formed from the reactants equals the
More informationHow To Calculate Mass In Chemical Reactions
We have used the mole concept to calculate mass relationships in chemical formulas Molar mass of ethanol (C 2 H 5 OH)? Molar mass = 2 x 12.011 + 6 x 1.008 + 1 x15.999 = 46.069 g/mol Mass percentage of
More informationINTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION. 37 74 20 40 60 80 m/e
CHM111(M)/Page 1 of 5 INTI COLLEGE MALAYSIA A? LEVEL PROGRAMME CHM 111: CHEMISTRY MOCK EXAMINATION: DECEMBER 2000 SESSION SECTION A Answer ALL EIGHT questions. (52 marks) 1. The following is the mass spectrum
More information1 Exercise 2.19a pg 86
In this solution set, an underline is used to show the last significant digit of numbers. For instance in x = 2.51693 the 2,5,1, and 6 are all significant. Digits to the right of the underlined digit,
More informationSample Exercise 8.1 Magnitudes of Lattice Energies
Sample Exercise 8.1 Magnitudes of Lattice Energies Without consulting Table 8.2, arrange the following ionic compounds in order of increasing lattice energy: NaF, CsI, and CaO. Analyze: From the formulas
More informationInstructions Answer all questions in the spaces provided. Do all rough work in this book. Cross through any work you do not want to be marked.
GCSE CHEMISTRY Higher Tier Chemistry 1H H Specimen 2018 Time allowed: 1 hour 45 minutes Materials For this paper you must have: a ruler a calculator the periodic table (enclosed). Instructions Answer all
More informationStoichiometry Exploring a Student-Friendly Method of Problem Solving
Stoichiometry Exploring a Student-Friendly Method of Problem Solving Stoichiometry comes in two forms: composition and reaction. If the relationship in question is between the quantities of each element
More informationQ1. A student studied the reaction between dilute hydrochloric acid and an excess of calcium carbonate.
Q. A student studied the reaction between dilute hydrochloric acid and an excess of calcium carbonate. calcium carbonate + hydrochloric acid calcium chloride + water + carbon dioxide The student measured
More informationChapter 6 An Overview of Organic Reactions
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 6 An Overview of Organic Reactions Why this chapter? To understand organic and/or biochemistry, it is necessary to know: -What occurs -Why and
More informationMeasuring volume of gas produced Measuring precipitation (because sulphur is produced) e.g. look for X to disappear Measure mass lost
Introduction My investigation is about the rate of reaction. A rate of reaction is defined as how fast or slow a reaction takes place. For example, the oxidation of iron under the atmosphere is a slow
More informationChemistry 132 NT. Solubility Equilibria. The most difficult thing to understand is the income tax. Solubility and Complex-ion Equilibria
Chemistry 13 NT The most difficult thing to understand is the income tax. Albert Einstein 1 Chem 13 NT Solubility and Complex-ion Equilibria Module 1 Solubility Equilibria The Solubility Product Constant
More information1. Oxidation number is 0 for atoms in an element. 3. In compounds, alkalis have oxidation number +1; alkaline earths have oxidation number +2.
à xidation numbers In the Lewis model of bonding, when nonidentical atoms are bonded together, an important consideration is how the bonding electrons are apportioned between the atoms. There are two different
More informationChemistry 122 Mines, Spring 2014
Chemistry 122 Mines, Spring 2014 Answer Key, Problem Set 9 1. 18.44(c) (Also indicate the sign on each electrode, and show the flow of ions in the salt bridge.); 2. 18.46 (do this for all cells in 18.44
More informationSteady state approximation
Steady state approximation Supplementary notes for the course Chemistry for Physicists Course coordinator: Prof. Dr. Mathias Nest Teaching assistant: Dr. Raghunathan Ramakrishnan contact: rama@mytum.de,
More informationUpon completion of this lab, the student will be able to:
1 Learning Outcomes EXPERIMENT B4: CHEMICAL EQUILIBRIUM Upon completion of this lab, the student will be able to: 1) Analyze the absorbance spectrum of a sample. 2) Calculate the equilibrium constant for
More informationMeasuring Protein Concentration through Absorption Spectrophotometry
Measuring Protein Concentration through Absorption Spectrophotometry In this lab exercise you will learn how to homogenize a tissue to extract the protein, and then how to use a protein assay reagent to
More informationEnzymes: Amylase Activity in Starch-degrading Soil Isolates
Enzymes: Amylase Activity in Starch-degrading Soil Isolates Introduction This week you will continue our theme of industrial microbiologist by characterizing the enzyme activity we selected for (starch
More informationChemical Composition. Introductory Chemistry: A Foundation FOURTH EDITION. Atomic Masses. Atomic Masses. Atomic Masses. Chapter 8
Introductory Chemistry: A Foundation FOURTH EDITION by Steven S. Zumdahl University of Illinois Chemical Composition Chapter 8 1 2 Atomic Masses Balanced equation tells us the relative numbers of molecules
More information7. 1.00 atm = 760 torr = 760 mm Hg = 101.325 kpa = 14.70 psi. = 0.446 atm. = 0.993 atm. = 107 kpa 760 torr 1 atm 760 mm Hg = 790.
CHATER 3. The atmosphere is a homogeneous mixture (a solution) of gases.. Solids and liquids have essentially fixed volumes and are not able to be compressed easily. have volumes that depend on their conditions,
More informationACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND
#3. Acid - Base Titrations 27 EXPERIMENT 3. ACID-BASE TITRATIONS: DETERMINATION OF CARBONATE BY TITRATION WITH HYDROCHLORIC ACID BACKGROUND Carbonate Equilibria In this experiment a solution of hydrochloric
More informationAcids and Bases HW PSI Chemistry
Acids and Bases HW PSI Chemistry Name 1) According to the Arrhenius concept, an acid is a substance that. A) is capable of donating one or more H + B) causes an increase in the concentration of H + in
More informationCh 20 Electrochemistry: the study of the relationships between electricity and chemical reactions.
Ch 20 Electrochemistry: the study of the relationships between electricity and chemical reactions. In electrochemical reactions, electrons are transferred from one species to another. Learning goals and
More information1.3.1 Position, Distance and Displacement
In the previous section, you have come across many examples of motion. You have learnt that to describe the motion of an object we must know its position at different points of time. The position of an
More information1. The graph below represents the potential energy changes that occur in a chemical reaction. Which letter represents the activated complex?
1. The graph below represents the potential energy changes that occur in a chemical reaction. Which letter represents the activated complex? 4. According to the potential energy diagram shown above, the
More informationChemical Equations & Stoichiometry
Chemical Equations & Stoichiometry Chapter Goals Balance equations for simple chemical reactions. Perform stoichiometry calculations using balanced chemical equations. Understand the meaning of the term
More information2 Spectrophotometry and the Analysis of Riboflavin
2 Spectrophotometry and the Analysis of Riboflavin Objectives: A) To become familiar with operating the Platereader; B) to learn how to use the Platereader in determining the absorption spectrum of a compound
More informationEXPERIMENT 11 UV/VIS Spectroscopy and Spectrophotometry: Spectrophotometric Analysis of Potassium Permanganate Solutions.
EXPERIMENT 11 UV/VIS Spectroscopy and Spectrophotometry: Spectrophotometric Analysis of Potassium Permanganate Solutions. Outcomes After completing this experiment, the student should be able to: 1. Prepare
More informationThermodynamics. Thermodynamics 1
Thermodynamics 1 Thermodynamics Some Important Topics First Law of Thermodynamics Internal Energy U ( or E) Enthalpy H Second Law of Thermodynamics Entropy S Third law of Thermodynamics Absolute Entropy
More informationChemical Equations. Chemical Equations. Chemical reactions describe processes involving chemical change
Chemical Reactions Chemical Equations Chemical reactions describe processes involving chemical change The chemical change involves rearranging matter Converting one or more pure substances into new pure
More informationCurrent Staff Course Unit/ Length. Basic Outline/ Structure. Unit Objectives/ Big Ideas. Properties of Waves A simple wave has a PH: Sound and Light
Current Staff Course Unit/ Length August August September September October Unit Objectives/ Big Ideas Basic Outline/ Structure PS4- Types of Waves Because light can travel through space, it cannot be
More informationSolving Spectroscopy Problems
Solving Spectroscopy Problems The following is a detailed summary on how to solve spectroscopy problems, key terms are highlighted in bold and the definitions are from the illustrated glossary on Dr. Hardinger
More informationThe Determination of an Equilibrium Constant
The Determination of an Equilibrium Constant Computer 10 Chemical reactions occur to reach a state of equilibrium. The equilibrium state can be characterized by quantitatively defining its equilibrium
More informationFORM A is EXAM II, VERSION 1 (v1) Name
FORM A is EXAM II, VERSION 1 (v1) Name 1. DO NOT TURN THIS PAGE UNTIL DIRECTED TO DO SO. 2. These tests are machine graded; therefore, be sure to use a No. 1 or 2 pencil for marking the answer sheets.
More informationUsing the Spectrophotometer
Using the Spectrophotometer Introduction In this exercise, you will learn the basic principals of spectrophotometry and and serial dilution and their practical application. You will need these skills to
More informationIMPORTANT INFORMATION: S for liquid water is 4.184 J/g degree C
FORM A is EXAM II, VERSION 2 (v2) Name 1. DO NOT TURN THIS PAGE UNTIL DIRECTED TO DO SO. 2. These tests are machine graded; therefore, be sure to use a No. 1 or 2 pencil for marking the answer sheets.
More informationAn acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
Chapter 8 Acids and Bases Definitions Arrhenius definitions: An acid is a substance that produces H + (H 3 O + ) Ions in aqueous solution. A base is a substance that produces OH - ions in aqueous solution.
More informationChapter 3: Stoichiometry
Chapter 3: Stoichiometry Key Skills: Balance chemical equations Predict the products of simple combination, decomposition, and combustion reactions. Calculate formula weights Convert grams to moles and
More informationKinetic Mechanisms Why does a reaciton follow a particular rate law? What is actually happening in the reaction?
Today Kinetic Mechanisms Why does a reaciton follow a particular rate law? What is actually happening in the reaction? Transition State Theory Arrhenius Theory What is the rate law for the following reaction?
More informationLaboratory 5: Properties of Enzymes
Laboratory 5: Properties of Enzymes Technical Objectives 1. Accurately measure and transfer solutions with pipettes 2. Use a Spectrophotometer to study enzyme action. 3. Properly graph a set of data. Knowledge
More informationSummer Holidays Questions
Summer Holidays Questions Chapter 1 1) Barium hydroxide reacts with hydrochloric acid. The initial concentration of the 1 st solution its 0.1M and the volume is 100ml. The initial concentration of the
More informationChemistry 12 Worksheet 1-1 - Measuring Reaction Rates
Chemistry 12 Worksheet 1-1 - Measuring Reaction Rates 1. A chemist wishes to determine the rate of reaction of zinc with hydrochloric acid. The equation for the reaction is: Zn (s) + 2HCl (aq) oh 2(g)
More information1. How many hydrogen atoms are in 1.00 g of hydrogen?
MOLES AND CALCULATIONS USING THE MOLE CONCEPT INTRODUCTORY TERMS A. What is an amu? 1.66 x 10-24 g B. We need a conversion to the macroscopic world. 1. How many hydrogen atoms are in 1.00 g of hydrogen?
More informationMelting Range 1 Experiment 2
Melting Range 1 Experiment 2 Background Information The melting range of a pure organic solid is the temperature range at which the solid is in equilibrium with its liquid. As heat is added to a solid,
More informationName Partners Date. Energy Diagrams I
Name Partners Date Visual Quantum Mechanics The Next Generation Energy Diagrams I Goal Changes in energy are a good way to describe an object s motion. Here you will construct energy diagrams for a toy
More informationHEAT UNIT 1.1 KINETIC THEORY OF GASES. 1.1.1 Introduction. 1.1.2 Postulates of Kinetic Theory of Gases
UNIT HEAT. KINETIC THEORY OF GASES.. Introduction Molecules have a diameter of the order of Å and the distance between them in a gas is 0 Å while the interaction distance in solids is very small. R. Clausius
More informationChapter 22 Carbonyl Alpha-Substitution Reactions
John E. McMurry www.cengage.com/chemistry/mcmurry Chapter 22 Carbonyl Alpha-Substitution Reactions The α Position The carbon next to the carbonyl group is designated as being in the α position Electrophilic
More informationStudy the following diagrams of the States of Matter. Label the names of the Changes of State between the different states.
Describe the strength of attractive forces between particles. Describe the amount of space between particles. Can the particles in this state be compressed? Do the particles in this state have a definite
More informationCandidate Style Answer
Candidate Style Answer Chemistry A Unit F321 Atoms, Bonds and Groups High banded response This Support Material booklet is designed to accompany the OCR GCE Chemistry A Specimen Paper F321 for teaching
More informationGuide to Chapter 13. Chemical Equilibrium
Guide to Chapter 13. Chemical Equilibrium We will spend five lecture days on this chapter. During the first class meeting we will focus on how kinetics makes a segue into equilibrium. We will learn how
More informationKinetic studies using UV-VIS spectroscopy Fenton reaction
Kinetic studies using UV-VIS spectroscopy Fenton reaction Abstract The goal of this exercise is to demonstrate the possibility of using a modern in situ spectroscopic method (UV-VIS spectroscopy) to investigate
More informationChapter 1: Moles and equations. Learning outcomes. you should be able to:
Chapter 1: Moles and equations 1 Learning outcomes you should be able to: define and use the terms: relative atomic mass, isotopic mass and formula mass based on the 12 C scale perform calculations, including
More informationAcids and Bases: A Brief Review
Acids and : A Brief Review Acids: taste sour and cause dyes to change color. : taste bitter and feel soapy. Arrhenius: acids increase [H ] bases increase [OH ] in solution. Arrhenius: acid base salt water.
More informationChemistry 111 Laboratory Experiment 7: Determination of Reaction Stoichiometry and Chemical Equilibrium
Chemistry 111 Laboratory Experiment 7: Determination of Reaction Stoichiometry and Chemical Equilibrium Introduction The word equilibrium suggests balance or stability. The fact that a chemical reaction
More informationSolubility Product Constant
Solubility Product Constant Page 1 In general, when ionic compounds dissolve in water, they go into solution as ions. When the solution becomes saturated with ions, that is, unable to hold any more, the
More informationChapter 11 Homework and practice questions Reactions of Alkyl Halides: Nucleophilic Substitutions and Eliminations
Chapter 11 Homework and practice questions Reactions of Alkyl Halides: Nucleophilic Substitutions and Eliminations SHORT ANSWER Exhibit 11-1 Circle your response in each set below. 1. Circle the least
More informationQ.1 Classify the following according to Lewis theory and Brønsted-Lowry theory.
Acid-base 2816 1 Acid-base theories ACIDS & BASES - IONIC EQUILIBRIA LEWIS acid electron pair acceptor H +, AlCl 3 base electron pair donor NH 3, H 2 O, C 2 H 5 OH, OH e.g. H 3 N: -> BF 3 > H 3 N + BF
More informationEXPERIMENT 7 Reaction Stoichiometry and Percent Yield
EXPERIMENT 7 Reaction Stoichiometry and Percent Yield INTRODUCTION Stoichiometry calculations are about calculating the amounts of substances that react and form in a chemical reaction. The word stoichiometry
More information2(H 2 O 2 ) catalase 2H 2 O + O 2
Enzyme Model Catalase Student Guide Catalysts accelerate chemical reactions that otherwise proceed slowly. The enzyme called catalase is a catalyst. It exists in plant and animal cells and breaks down
More information